- #1
Saba
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- TL;DR
- When sodium acetate CH3COONa reacts with water does it form hydroxide ions, leaving the neutralised solution alklain?
How does Sodium acetate react with water?
- Thread starter Saba
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Discussion Overview
The discussion centers on the reaction of sodium acetate with water, exploring the resulting chemical processes, particularly hydrolysis, and the implications for solution pH. The scope includes theoretical aspects of acid-base chemistry and the behavior of solutions at varying concentrations.
Discussion Character
- Exploratory, Technical explanation, Conceptual clarification
Main Points Raised
- One participant suggests that sodium acetate removes a proton from water, indicating that CH3COO- acts as the anion of a weak acid while Na+ is the cation of a strong base.
- Another participant confirms the hydrolysis process, providing a chemical equation that illustrates the reaction between CH3COO- and water, producing CH3COOH and OH-.
- A claim is made that a 0.01M solution of sodium acetate has a calculated pH of 8.4, suggesting that even low concentrations can lead to observable alkalinity in the solution.
- A later reply notes a perceived fading of precise knowledge regarding these concepts over the years, indicating a potential shift in understanding or teaching of the material.
Areas of Agreement / Disagreement
Participants generally agree on the occurrence of hydrolysis and the alkaline nature of sodium acetate solutions, though there is no consensus on the implications of knowledge changes over time.
Contextual Notes
Limitations include assumptions about concentration effects on pH and the potential variability in individual understanding of acid-base theory.
- #2
symbolipoint
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Removes a 'proton' from the water molecule. You might think of it like, CH3COO-is the anion of a weak acid and Na+ is the cation of a strong base. Sodium acetate dissolved in water would if conc. is high enough, make the solution alkaline.
- #3
Borek
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Congratulations, you just discovered process of hydrolysis 
Yes, that's what is happening:
CH3COO- + H2O ↔ CH3COOH + OH-
You might want to read on Brønsted–Lowry acid–base theory, this reaction is an important part of it.
Yes, that's what is happening:
CH3COO- + H2O ↔ CH3COOH + OH-
You might want to read on Brønsted–Lowry acid–base theory, this reaction is an important part of it.
- #4
Borek
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symbolipoint said:
0.01M solution of sodium acetate has a calculated pH of 8.4, you don't need high concentrations for the effect to be easily observable.
- #5
symbolipoint
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Some fading of precise knowledge has been happening the last several years. (That is, in my knowledge)Borek said:
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